CATALYSTS FOR ELECTROCHEMICAL CO2 REDUCTION AND ASSOCIATED METHODS

Description

TECHNICAL FIELD

[0001] The technical field generally relates to catalytic methods for CO₂ reduction, and more particularly to electrocatalysts composed of Cu-Al multi-metallic material and associated methods of manufacture and use in electrochemical CO₂ reduction.

BACKGROUND

[0002] The efficient electrochemical conversion of carbon dioxide (CO₂) into valuable carbon-based fuels and compounds is desirable and technology that enhances such conversion can, for example, enable the storage of intermittent renewable electricity as well as net reductions of greenhouse gas emissions. Copper has been the predominant electrocatalyst for the production of multi-carbon products. However, achieving high selectivity and productivity to certain desired chemicals (e.g., ethylene, a highly demanded industrial feedstock) has failed to meet requirements of practical operation (e.g., current density over 250 mA cm^-2, applied cell voltage below 3 V, Faradaic efficiency to one certain desired product at least above 70%).

[0003] US2018057950 describes methods for electrochemically reducing carbon dioxide to provide a product. The methods can comprise contacting the carbon dioxide with an electroreduction catalyst in an electrochemical cell, and applying a potential to the electrochemical ceil to form the product. The electroreduction catalyst can comprise a nanoporous Cu catalyst, a nanoporous Cu-M catalyst, or a combination thereof, where M is a metal chosen from Pt, Ir, Pd, Ag, Au, Rh, Ru, Zn, Sn, Ni, Fe, Re, Ga, In, Cd, Tl, and Ti. The product can comprise a C2-C3 alkane, a C2-C3 alkene, a C2-C3 alcohol, a C2-C3 carboxylic acid, a C2-C3 aldehyde, or a combination thereof.

[0004] AU2016305184 relates to a gas diffusion electrode comprising a, preferably copper-containing, carrier and a first layer having at least copper and at least one binder, wherein the first layer has hydrophilic and hydrophobic pores and/or channels, further comprising a second layer having copper and at least one binder, wherein the second layer is located on the carrier and the first layer is located on the second layer, wherein the binder content in the first layer is less than in the second layer. This document further relates to a method for producing a gas diffusion electrode of this type and an electrolysis cell comprising a gas diffusion electrode of this type.

[0005] US2015056385 is about a Cu wiring structure forming method. In such a method, a barrier film serving as a Cu diffusion barrier is formed at least on a surface of a recess in a first insulating film formed on a substrate, and the recess is filled with an Al-containing Cu film. A Cu wiring is formed from the Al-containing Cu film, and a cap layer including a Ru film is formed on the Cu wiring. Further, an interface layer containing a Ru-AI alloy is formed at an interface between the Cu wiring and the cap layer by heat generated in forming the cap layer or by a heat treatment performed after forming the cap layer. A second insulating film is formed on the cap layer.

[0006] There is a need for improved techniques and catalyst materials for efficient electrochemical CO₂ reduction and related methods and systems of producing chemical compounds.

SUMMARY

[0007] Multi-metal electrocatalysts for reduction of CO₂ to produce multi-carbon compounds can include Cu and at least one metal selected from Ge, Ga, Sn, Si, Ag, Au, Zn and Al. With preference, they include a Cu-Al material that may be de-allowed and formed as a catalytic layer on a gas diffusion membrane. The multi-metal Cu-Al material can include 1 wt% to 50 wt% Al and 50 wt% to 99 wt% Cu, for example. The Al can be ion-implanted into the Cu or Al can be evaporated into the Cu and remains after chemical etching. The electrocatalyst can have a surface region that is nanoporous. Other multi-metal electrocatalyst compositions are also possible. The electrocatalysts can have various properties, structural features, chemical compositions and their chemical states as will be described in detail further below.

[0008] The electrocatalysts can be implemented in electrocatalytic reduction of CO₂ into at least one multi-carbon compound, such as ethylene. The electrocatalytic reduction of CO₂ can be performed in an alkaline medium, such as potassium hydroxide.

[0009] The electrocatalysts can be manufactured by vapour-phase deposition of Al onto a Cu surface and chemically etching the metallic alloy to produce a de-alloyed Cu-Al material, or by ion-implanting Al into Cu, for example.

[0010] The electrocatalysts and associated methods and uses have been found to provide advantageous functionality related to the production of electrocatalytic reduction of CO₂ into multi-carbon compounds.

[0011] Therefore, according to a first aspect, the invention provides for an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, remarkable in that the electrocatalyst comprises a multi-metal material comprising a primary metal being copper (Cu) and at least one enhancer metal being aluminium (Al), so the electrocatalyst comprises a multi-metal Cu-Al material being formed as a catalytic layer and comprises a surface region having a thickness between 1 nm and 3 nm as determined by Auger electron spectroscopy and in that at least the surface region is nanoporous and comprises an Al content of 3 wt% to 30 wt% and a Cu content of 70 wt% to 97 wt%..

[0012] In a preferred embodiment, the invention provides for an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, remarkable in that the electrocatalyst comprises a multi-metal Cu-Al material. With preference, the multi-metallic Cu-Al material consists of Cu and Al.

[0013] Surprisingly, the Inventors have found a new CO₂ electroreduction Cu-based catalyst, such as comprising a Cu-Al multi-metal material with varying ratios of Al concentrations on surface, that shows superior CO₂ electroreduction activity to valuable multi-carbon products (e.g. ethylene).

[0014] The inventors then developed a physical vapor deposition and chemical etching process to scalably fabricate nanoporous Cu-Al catalysts that enable highly selective production of ethylene with a record CO₂-to-ethylene Faradaic efficiency of 80% at an unprecedently high applied current density of 600 mA cm^-2 (-1.8 to -2.1 V vs. RHE) in a flow cell system. This result vastly improves the CO₂-to-ethylene selectivity and stability with a fairly high half-cell electricity-to-ethylene power conversion efficiency of 30% which readily meets the requirements of practical operation.

[0015] The inventors find out that Cu-Al alloys provide multiple sites and surface orientations that exhibit optimal CO adsorption energies near the top of the activity volcano plot for CO₂ reduction. In situ X-ray absorption further reveals how Cu and Al enable a favourable Cu coordination environment that enhances C-C dimerization, the rate-determining step from CO₂ to C2 products.

[0016] With preference, the one or more following features can be used to further define the multi-metal Cu-Al material:

• The multi-metal Cu-Al material is a de-alloyed Cu-Al material.
• The multi-metal Cu-Al material comprises from 1 wt% to 50 wt% of Al based on the total weight of the multi-metal Cu-Al material, preferably from 2 wt% to 40 wt% of Al, more preferably from 3 wt% to 30 wt% of Al.
• The multi-metal Cu-Al material comprises from 50 wt% to 99 wt% of Cu, based on the total weight of the multi-metal Cu-Al material, preferably from 80 wt% to 98 wt%, more preferably from 70 wt% to 97 wt% Cu.

[0017] In an embodiment, the multi-metal Cu-Al material comprises Cu doped with Al. In another embodiment, the multi-metal Cu-Al material comprises Al doped with Cu.

[0018] With preference:

• the electrocatalyst comprises a gas diffusion membrane; and/or
• the catalytic layer is formed directly on a gas diffusion membrane; and/or
• the catalytic layer has a thickness between 1 nm and 5000 nm as determined by cross-sectional scanning electron microscopy; preferably 10 to 5000 nm.

[0019] The invention uses thermal evaporation or co-sputtering to deposit the catalyst layer on the gas diffusion membrane. For the thermal evaporation, the thickness of the catalyst layer is monitored with a film-thickness sensor during the deposition. For the co-sputtering, the depositing rate of each catalyst material is first measured by depositing it on flat Si substrates under the same deposition conditions used for depositing the catalyst layer on the gas diffusion membrane. Once the deposition rate of each material is known, the film thickness can be controlled by its deposition time.

[0020] The thickness of the catalytic layer can also be determined by cross-sectional scanning electron microscopy (SEM).

[0021] One or more of the following features can be used to better define the catalyst layer:

• The catalyst layer has a thickness ranging between 10 and 1500 nm as determined by cross-sectional scanning electron microscopy (SEM)
• The catalyst layer has a thickness of at least 15 nm as determined by cross-sectional scanning electron microscopy (SEM), preferably at least 50 nm, and more preferably of at least 100 nm.
• The catalyst layer has a thickness of at most 1200 nm as determined by cross-sectional scanning electron microscopy (SEM), preferably of at most 1000 nm, and more preferably of at most and 500 nm.

[0022] According to the invention the Cu-Al catalyst can be of two types:

• In a first embodiment, the multi-metal Cu-Al material used as Cu-Al catalyst is produced by first depositing Cu-Al alloy on a gas diffusion layer and then de-alloying the Cu-Al alloy by chemical etching. After de-alloying, the multi-metal Cu-Al catalyst is in a porous structure. A certain amount of Al (1-50 wt% Al, 3-30 wt% Al in the optimal case) is present on the catalyst surface.
• In a second embodiment, the multi-metal Cu-Al material used as Cu-Al catalyst is produced by first depositing a Cu catalyst layer on a gas diffusion layer and then ion-implanting Al into the Cu layer to make a Cu-Al surface.

[0023] In a preferred embodiment, the Cu and Al in the multi-metal Cu-Al material are morphologically stable after five hours of electroreduction reaction in alkaline electrolyte.

[0024] With preference, Al concentration in the multi-metal Cu-Al material is stable after five hours of electroreduction reaction in alkaline electrolyte.

[0025] The multi-metal Cu-Al catalyst is both morphologically and compositionally stable after five hours of electroreduction reaction in the alkaline electrolyte. The Cu-Al material shows a very similar porous morphology with pore diameters of 5-50 nm before and after the chemical reaction in the alkaline electrolyte. The Cu and Al concentrations on the Cu-Al catalyst surface is almost unchanged (concentration variation within 5 wt%) before and after the chemical reaction.

[0026] With preference, one or more of the following is true:

• At least the surface region consists of Cu and Al.
• At least the surface region has pores that have pore diameters ranging from 1 nm to 100 nm, or from 5 nm to 20 nm as determined HRTEM and HAADF analysis.
• At least the surface region has a homogeneous distribution of Al and Cu.

[0027] In a preferred embodiment, the Cu in at least the surface region is Cu (111); with preference, the Al content in the Cu (111) is about 8 wt% to about 15 wt%, or about 11 wt% to about 13 wt%.

[0028] In another embodiment, the Cu in at least the surface region is Cu (100); with preference, the Al content in the Cu (100) is about 3 wt% to about 15 wt%.

[0029] With preference, the enhancer metal increases catalytic site density with decreased reaction energy for the C-C dimerization; with preference, the reaction energy for the C-C dimerization is decreased by 0.3 eV to 0.7 eV.

[0030] With preference, the multi-metal material comprises enhancer metal-terminated pores.

[0031] According to a second aspect, the invention provides the use of the electrocatalyst as defined in the first aspect, for electrocatalytic reduction of CO₂ into at least one multi-carbon compound. Preferably, the at least one multi-carbon compound comprises ethylene.

[0032] In a preferred embodiment, the electrocatalytic reduction of CO₂ is performed in an alkaline medium; with preference, the alkaline medium comprises potassium hydroxide.

[0033] In a further preferred embodiment, the electrocatalytic reduction of CO₂ is performed in a three-electrode flow-cell.

[0034] According to a third aspect, the invention provides a process for electrochemical production of a multi-carbon compound from CO₂, comprising:

• contacting CO₂ gas and an electrolyte with an electrode comprising the electrocatalyst as defined in any one of the first aspect such that the CO₂ contacts the electrocatalyst;
• applying a voltage to provide a current density to cause the CO₂ gas contacting the electrocatalyst to be electrochemically converted into the multi-carbon compound; and
• recovering the multi-carbon compound.

[0035] The one or more following features can be further used to further define the process according to the third aspect:

• The current density provided in the current collection structure is predetermined for selective electrochemical conversion of the CO₂ into a target multi-carbon compound.
• The target multi-carbon compound is ethylene or an alcohol.
• The electrolyte comprises an alkaline compound.
• The electrolyte comprises KOH and/or other alkaline solutions.
• The process is conducted in a three-electrode flow-cell.

[0036] According to a fourth aspect, the invention provides a system for CO₂ electroreduction to produce multi-carbon hydrocarbons, comprising:

• an electrolytic cell configured to receive a liquid electrolyte and CO₂ gas;
• an anode;
• a cathode comprising an electrocatalyst as defined in any one of the first aspect and
• a voltage source to provide a current density to cause the CO₂ gas contacting the electrocatalyst to be electrochemically converted into the multi-carbon hydrocarbon, which is optionally ethylene or an alcohol.

[0037] According to a fifth aspect, the invention provides a method of manufacturing the electrocatalyst as defined in any one of the first aspect comprising vapour-phase deposition followed by chemical etching or ion-implanting.

[0038] According to an sixth aspect, the invention provides a method of manufacturing an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, the method comprising:

• producing a metallic material comprising Cu and Al; and
• subjecting the metallic material to chemical etching to remove a portion of the Al from a surface region of the metallic alloy to produce a de-alloyed Cu-Al material.

[0039] In a preferred embodiment, the method comprises producing the metallic material comprises vapour-phase deposition of Al onto a Cu surface; with preference:

• the vapour-phase deposition comprising evaporating solid Al and forming a deposited Al layer on the Cu surface to form an evaporated AI-on-Cu material.
• the deposited Al layer has a thickness of about 50 to 150 nm as determined by cross-sectional scanning electron microscopy.
• the evaporating of the solid Al is performed at an evaporation rate of approximately 1-10 nm s^-1, 1-5 nm s^-1 or 1-2 nm s^-1.
• the evaporating of the solid Al is performed at under a base pressure of about 10^-5 to 10^-8 Torr (133.32 × 10^-5 to 133.32 × 10^-8 Pa).

[0040] In a preferred embodiment, the method comprises producing the metallic material comprises vapour-phase deposition of Al onto a Cu surface; with preference:

• the chemical etching comprises immersing the evaporated Al-on-Cu material into an acidic solution to remove Al.
• the acidic solution comprises hydrochloric acid solution.
• the hydrochloric acid solution comprises from 1 to 20 wt% of hydrochloric acid, preferably from 1 to 10 wt% of hydrochloric acid, more preferably from 1 to 5 wt% hydrochloric acid.
• The method further comprising, after chemical etching, washing with water to remove the acidic solution; with preference, further comprising, after washing, air drying to remove water.
• The method further comprising, prior to producing the metallic alloy comprising the Cu and Al, depositing Cu on a gas diffusion layer (GDL).
• the Cu is deposited by thermal evaporation onto the GDL.
• the Cu forms a deposited Cu layer on the GDL.
• the deposited Cu layer has a thickness of about 400 to 600 nm as determined by cross-sectional scanning electron microscopy.

[0041] In a preferred embodiment, producing the metallic material comprises co-evaporation of Al and Cu to form a Cu-Al alloy; with preference:

• The method further comprises depositing a layer of the Cu-Al alloy onto a gas diffusion layer (GDL) prior to the chemical etching.
• The method further comprises cooling the deposited Cu-Al alloy prior to chemical etching.
• The chemical etching comprises immersing the Cu-Al alloy in an acidic solution to remove Al; preferably, the acidic solution comprises hydrochloric acid solution, and/or the method further comprises, after chemical etching, washing with water to remove the acidic solution.

[0042] According to a seventh aspect, the invention provides a method of manufacturing an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, the method comprising ion-implanting Al into Cu.

DESCRIPTION OF FIGURES

[0043] 

Figure 1: Screening of Cu and Cu based compounds using computational methods. a, DFT-calculated CO adsorption energies (ΔE_co) of the surfaces. Energies are plotted on a volcano-shaped scaling relationship. Random noise was added to the (ΔE_co) values to distinguish different points more effectively. b, t-SNE representation of 3,494 adsorption sites that the method performed DFT calculations on. All Cu-Al clusters are labelled numerically. c, Representative coordination sites for each of the clusters labelled in the t-SNE diagram.

Figure 2: Schematic and characterization of de-alloyed Cu-Al catalyst, a, Schematic of a de-alloyed nanoporous Cu-Al catalyst on a gas diffusion layer for CO₂ electroreduction. b, Scanning electron microscopy (SEM) and high angle angular dark field-scanning transmission electron microscopy (HAADF-STEM) images of de-alloyed Cu-Al catalyst before (left) and after (right) 5 hours CO₂ electroreduction at an applied current density of 600 mA cm^-2 in flow cells. The scale bars for SEM images are 500 nm (top-left) and 200 nm (top-right). The scale bars for TEM images are 200 nm (bottom-left) and 100 nm (bottom-right). c, HAADF-STEM image, and electron energy loss spectroscopy (EELS) spectra of the de-alloyed Cu-Al catalyst. #1, 2, 3 curves in the EELS spectra represent the EELS results measured at #1, 2, 3 areas in the corresponding HAADF-STEM image. Al, Al₂O₃, CuO, Cu₂O and Cu EELS results are plotted as references. The scale bar is 5 nm.

Figure 3: Analyses of (111) and (100) facets across varying ratios of Al concentrations. a, b, The distribution of ΔE_co values for the adsorption sites on Cu (111) and (100) surfaces with different amounts of Al replacement on the top layer of atoms.

Figure 4: CO₂ electroreduction performance on de-alloyed Cu-Al, porous Cu and deposited Cu catalysts. a, Faradaic efficiencies for gaseous products with de-alloyed Cu-Al catalysts at different applied current densities and with nanoporous Cu and evaporated Cu catalysts at a constant current density of 600 mA cm^-2 obtained using chronopotentiometry. b, Faradaic efficiencies for all products at an applied current density of 600 mA cm^-2 with 17 de-alloyed Cu-AI samples measured. c, Current-potential curves with de-alloyed Cu-Al, nanoporous Cu and evaporated Cu catalysts obtained from linear sweep voltammetry scans. d, C₂H₄ production partial current density vs. potential with de-alloyed Cu-Al, nanoporous Cu and evaporated Cu catalysts. e, The CO₂ electroreduction activity of a de-alloyed Cu-Al catalyst at an applied current density of 600 mA cm^-2. Left axis: potential (V vs. RHE) vs. time (s), right axis: C₂H₄ Faradaic efficiency (%) vs. time (s).

Figure 5: a, Faradaic efficiencies of CO₂ reduction to CO, H₂, CH₄ and C₂H₄ with Cu, Al-on-Cu (ion implant) and Al-on-Cu (evap. + etch); b, C₂H₄ partial current density versus potential with Cu, Al-on-Cu (ion implant) and Al-on-Cu (evap. + etch); c, SEM images of Al-on-Cu (ion implant) before and after 5 hours CO₂ RR reaction; d, SEM images of Al-on-Cu (evap. + etch) before and after 5 hours CO₂ RR reaction.

Figure 6: a, Faradaic efficiencies of CO₂ reduction to CO, H₂, CH₄ and C₂H₄ with de-alloyed Cu-Al at different current densities and with porous Cu and Cu at 600 mA cm^-2; b, Faradaic efficiency of CO₂ reduction to CO, H₂, CH₄, C₂H₄, C₂H₅OH, formic, n-propanol with de-alloyed Cu-Al; c, CO₂ reduction activity of de-alloyed Cu-Al at 600 mA cm^-2; d, SEM, TEM and EDX images of de-alloyed Cu-Al before and after 5 hours CO₂ RR reaction.

Figure 7: a-b, In situ X-ray absorption near-edge structure (XANES) spectra of de-alloyed Cu-AI catalyst before, during and after CO₂ electroreduction tests and ex-situ XANES spectra of Cu foil, Cu₂O, CuO. c-d, In situ X-ray absorption near-edge structure (XANES) spectra of pure Cu catalyst before and during CO₂ electroreduction tests and ex-situ XANES spectra of Cu foil.

Figure 8: Schematic for the synthesis of different catalysts on gas diffusion layers. a, evaporated Cu. b, ion-implanted Al-on-Cu. c, evaporated-etched Al-on-Cu. d, de-alloyed Cu-AI catalysts.

Figure 9: Morphologies of evaporated Cu catalysts on gas diffusion layers. a, Top-view SEM images before CO₂ electroreduction. b, Top-view SEM images after 5 hours CO₂ electroreduction in 1 M KOH at an applied current density of 600 mA cm^-2 in a flow cell.

Figure 10: Morphologies of ion-implanted Al-on-Cu catalysts on gas diffusion layers. a, Top-view SEM images before CO₂ electroreduction. b, Top-view SEM images after 5 h CO₂ electroreduction in 1 M KOH at an applied current density of 600 mA cm^-2 in a flow cell.

Figure 11: Morphologies of evaporated and evaporated-etched Al-on-Cu samples on gas diffusion layers. a, Top-view SEM images of the as-evaporated Al-on-Cu samples. b, Top-view SEM images of the evaporated-etched Al-on-Cu catalyst before CO₂ electroreduction, c

Figure 12: Schematic of the cathode side in a flow-cell configuration.

Figure 13: CO₂ electroreduction performances on pure Cu, ion-implanted Al-on-Cu, and evaporated-etched Al-on-Cu catalysts. a, Faradaic efficiencies of gaseous products on pure Cu, ion-implanted, and evaporated-etched Al-on-Cu obtained from chronopotentiometry tests at an applied current density of 600 mA cm^-2. b, C₂H₄ production partial current density versus potential on pure Cu, ion-implanted, and evaporated-etched Al-on-Cu.

Figure 14: Auger electron spectroscopic analysis of an ion-implanted Al-on-Cu catalyst, a, Auger secondary electron microscopic image. b, Auger spectroscopic narrow-scan spectra. c, Concentrations of Cu and Al.

Figure 15: Auger electron spectroscopic analysis of an evaporated-etched Al-on-Cu catalyst.

a, Auger secondary electron microscopic image. b, Auger spectroscopic narrow-scan spectra.

c, Concentrations of Cu and Al.

Figure 16: Pourbaix diagrams. Pourbaix diagrams of a, Cu and b, Al at ionic concentrations of 1 µM. The potentials versus the standard hydrogen electrode (V vs. SHE) can be converted to the reversible hydrogen electrode scale (V vs. RHE) according to the Nernst equation, V vs.

RHE = V vs. SHE + 0.059 × pH.

Figure 17: EDX analysis of an as-prepared ion-implanted Al-on-Cu sample before CO₂ electroreduction. a, Elemental concentrations.

Figure 18: EDX analysis of an ion-implanted Al-on-Cu sample after 5 hours CO₂ electroreduction. a, Elemental concentrations. Potassium is observed on the surface after the reaction.

Figure 19: EDX analysis of an evaporated-etched Al-on-Cu sample before CO₂ electroreduction. a, EDX mapping. b, Elemental concentrations. Chlorine is observed on the surface due to the use of HCl solution in the etching process.

Figure 20: EDX analysis of an evaporated-etched Al-on-Cu sample after 5 hours CO₂ electroreduction. a, EDX mapping. b, Elemental concentrations. Potassium was observed on the surface after the reaction.

Figure 21: EDX analysis of a pure Cu catalyst after half-hour CO₂ electroreduction in 1 M KOH with 1 mM Al(OH)₄^-. a, EDX mapping. b, Elemental concentrations. Fluorine was from the PTFE/carbon layer in the gas diffusion electrode. Al was electrodeposited on Cu at an applied current density of 600 mA cm^-2. Therefore, dissolving Al into solution was avoided.

Figure 22: Auger electron spectroscopic analysis of a pure Cu catalyst after 0.5-hour CO₂ electroreduction at 600 mA cm^-2 in 1 M KOH with 1 mM Al(OH)^-. a, Auger secondary electron microscopic image. b, Auger spectroscopic narrow-scan spectra. c, Concentrations of Cu and Al.

Figure 23: CO₂ electroreduction performance. Faradaic efficiencies for gaseous products with a pure Cu catalyst at a constant current density of 600 mA cm^-2 in 1 M KOH with the presence of 1 mM Al(OH)₄^- obtained from Chronopotentiometry tests.

Figure 24: EDX analysis of a pure Cu after immersing in 1 M KOH with 1 mM Al(OH)4^- for 0.5 hour. a, EDX mapping. b, Elemental concentrations. The invention manually selected Al and it was automatically marked in red by EDX software (Esprit 2.1) with a large error of 43.81%, indicating Al was actually out of the EDX detecting limit. As shown in the SEM image in Figure 19a, the morphology was also drastically changed. Most of Cu dissolved into 1 M KOH leaving thin Cu(OH)₂ nanowires to be dissolved.

Figure 25: Top-view SEM images of the de-alloyed Cu-Al catalyst at different magnifications.

Figure 26: EDX analyses in TEM of de-alloyed Cu-Al catalysts. a, as-prepared de-alloyed Cu-AI catalyst, b, de-alloyed Cu-Al catalyst after 5 hours CO₂ electroreduction in 1 M KOH at 600 mA cm^-2 in a flow-cell configuration.

Figure 27: EDX analysis in SEM of the as-prepared de-alloyed Cu-Al catalyst before CO₂ electroreduction. a, EDX mapping. b, Elemental concentrations. Chlorine was detected because of the use of a 5 wt% HCl solution in the etching process to prepare a de-alloyed Cu-AI catalyst.

Figure 28: EDX analysis in SEM of a de-alloyed Cu-Al catalyst after 5 hours CO₂ electroreduction. a, EDX mapping. b, Elemental concentrations. Potassium was detected because of the use of KOH electrolyte in CO₂ electroreduction.

Figure 29: STEM-ADF image of the de-alloyed Cu-Al catalyst. The observation was performed in the same area where the EELS analysis study was performed

Figure 30: Auger electron spectroscopic analysis of an as-prepared de-alloyed Cu-Al catalyst. a, Auger secondary electron microscopic image. b, Auger spectroscopic narrow-scan spectra. c, Concentrations of Cu and Al.

Figure 31: Auger electron spectroscopic analysis of a de-alloyed Cu-Al catalyst after 5 hours CO₂ electroreduction at 600 mA cm^-2. a, Auger secondary electron microscopic image. b, Auger spectroscopic narrow-scan spectra. c, Concentrations of Cu and Al.

Figure 32: Reaction Gibbs free energy diagram. Reaction Gibbs free energy diagram from adsorbed CO₂ to OC₂H₄, an intermediate to C₂H₄, and to CHOCH₃, an intermediate to C₂H₅OH, on the pure Cu (111) surface (blue lines) and ML predicted 12% Al incorporated Cu (111) surface (red lines). The ML predicted structure of 12% Al incorporated Cu (111) is inserted in the lower left.

Figure 33: Reaction Gibbs free energy diagram. Reaction Gibbs free energy diagram from adsorbed CO₂ to OC₂H₄, an intermediate to C₂H₄, and to CHOCH₃, an intermediate to C₂H₅OH, on the pure Cu (100) surface (blue lines) and ML predicted 4% Al incorporated Cu (100) surface (red lines). The ML predicted structure of 4% Al incorporated Cu (111) is inserted in the lower left.

Figure 34: De-alloyed Cu-Al with different surface Al concentrations. a, SEM images of de-alloyed Cu-Al with different etching time. b, Al concentrations on surfaces determined by surface-sensitive Auger electron spectroscopic analysis. Surface Al concentrations could be roughly varied from 4-28% by controlling the etching time. c, Faradaic efficiencies of C2+ and C2+/C1 ration with de-alloyed catalysts at different surface Al concentrations.

Figure 35: Half-cell electricity-to-ethylene power conversion efficiencies with de-alloyed Cu-Al catalyst plotted at different current densities. The invention estimates the half-cell power conversion efficiency using the equation:

where

Figure 36: SEM images of a de-alloyed Cu-Al catalyst soaked in 10 mM CuCl₂ for 10 minutes. 10 minutes is an optimal time that the invention used to roughly maintain nanoporosity while replacing surface Cu with Al by the displacement reaction of 2Al + 3CuCl₂ → 2AlCl₃ + 3Cu. The invention also found that nanopores were gradually blocked by the precipitated Cu with a prolonged CuCl₂ treatment.

Figure 37: Auger electron spectroscopic analysis of a de-alloyed Cu-Al catalyst soaked in 10 mM CuCl₂ solution for 0.5 hour. a, Auger secondary electron microscopic image. b, Auger spectroscopic narrow-scan spectra. c, Concentrations of Cu and Al. The Al concentration calculated from Al narrow-scan spectrum is already close to the AES detecting limit.

Figure 38: CO₂ electroreduction performance. Faradaic efficiencies for all products at an applied current density of 600 mA cm^-2 obtained with of a de-alloyed Cu-Al catalyst after soaking in 10 mM CuCl₂ solution for 10 minutes.

DETAILED DESCRIPTION

[0044] Techniques described herein relate to enhanced catalyst materials that can be used for electrochemical CO₂ reduction and the production of multi-carbon compounds, and also to methods of manufacturing such catalyst materials.

[0045] Figure 1 highlights that Cu-Al shows improved CO binding energy for better C-C dimerization. Figure 5 reveals that ion-implanting Al into Cu shows a better CO₂-electrolysis performance than that of pure Cu. Figure 6 shows that de-alloyed Cu-Al catalysts has a better CO₂-electrolysis performance than that of pure Cu.

The electrocatalyst

[0046] The invention provides an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds. According to the invention, the electrocatalyst comprises a multi-metal material comprising a primary catalyst material and an enhancer material. The enhancer material is selected to modify the coordination of the primary catalyst material in order to enhance the C-C dimerization. The multi-carbon compounds preferably comprise, or consist of, ethylene.

[0047] According to the invention, the primary catalyst material is copper (Cu); and/or the enhancer material is aluminium (Al).

[0048] Therefore, the electrocatalyst comprises, or consist of, a multi-metal Cu-Al material. Indeed, the new Cu-Al based electrocatalyst materials according to the invention demonstrate highly activity for electrochemical reduction of carbon dioxide to chemicals (e.g., ethylene).

[0049] In a preferred embodiment, in the multi-metal material, the primary catalyst material, preferably comprising Cu or consisting of Cu, is predominant. Thus, the multi-metal material comprises from 70 wt% to 97 wt% of the primary catalyst material, based on the total weight of the multi-metal material.

[0050] In a preferred embodiment, the multi-metal material the enhancer material, preferably comprising Al or consisting of Al, is present in a weight percentage that is inferior to the weight percentage of the primary catalyst material. Thus, the multi-metal material comprises from 3 wt% to 30 wt% of the enhancer material, based on the total weight of the multi-metal material..

[0051] In another embodiment, the multi-metal material is formed as a catalytic layer. Therefore, the invention provides an electrocatalyst comprising a catalytic layer and a gas diffusion membrane; wherein the catalytic layer has a thickness ranging from 10 nm to 5000 nm as determined by cross-sectional scanning electron microscopy; preferably from 2 nm to 2500 nm; more preferably from 3 nm to 1000 nm. With preference, the catalytic layer is formed directly on the gas diffusion membrane.

[0052] The gas diffusion membrane comprises a carbon-based material and/or is hydrophobic. In an embodiment, the gas diffusion membrane includes a hydrophobic polymer-based support such as polytetrafluoroethylene or similar polymers.

[0053] In an embodiment, the electrocatalyst described herein can be used as a catalyst layer in a composite multilayered electrocatalyst (CME) that includes a polymer-based gas-diffusion layer, a current collection structure, and the catalyst layer, sandwiched in between. The current collection structure can include a carbon nanoparticle layer applied against the catalyst layer, and a graphite layer applied against the nanoparticle layer. In one possible implementation of the CME, it includes hydrophobic polymer-based support such as polytetrafluoroethylene (PTFE); a Cu-Al or other multi-metal catalyst material deposited on top; a layer of carbon-based nanoparticles (NPs) atop the catalyst; and an ensuing layer of graphite as the electron conductive layer. In this configuration, the PTFE layer, which can be substantially pure PTFE or similar polymer, acts as a more stable hydrophobic gas-diffusion layer that prevents flooding from the catalyst; carbon NPs and graphite stabilize the metal catalyst surface; the graphite layer both serves as overall support and current collector. In an alternative implementation, the CME includes a hydrophobic polymer-based layer; the multi-metal electrocatalyst deposited on top; and then a layer of conductive material such as graphite deposited on top of the catalyst layer. In this configuration, the stabilization material (e.g., carbon nanoparticles) are not present as a distinct layer in between the graphite and the catalyst layers. Other features of the CME and related CO₂RR methods as described in the article Cao-Thang Dinh & al. "CO2 electroreduction to ethylene via hydroxide-mediated copper catalysis at an abrupt interface" Science 18 May 2018 Vol. 360, Issue 6390, pp. 783-787 (DOI: 10.1126 /science.aas 9100) can be used in combination with the electrocatalyst and methods described herein.

[0054] According to a preferred embodiment, the multi-metal material is a de-alloyed material. Thus, it is a de-alloyed Cu-Al material.

[0055] The structure of the multi-metal material can be as follow:

• the multi-metal material comprises enhancer material-terminated pores; or
• the enhancer material is ion-implanted into the primary catalyst material; or
• the enhancer material is present in the primary catalyst material as the enhancer material that has been evaporated into the primary catalyst material and remains after chemically etching

[0056] In an embodiment, the electrocatalyst is layered, and comprises an internal region and a surface region. The internal region may consist of the primary catalyst material or both of the primary catalyst material and the enhancer material. If the internal region consists of both the primary and enhance materials, their weight percentages can be varied from 1% - 99% for each.

[0057] The surface region of the electrocatalyst has preferably a thickness ranging between 1 nm to 3 nm as determined by Auger electron spectroscopy, preferably ranging from 1.5 to 2. 5 nm.

[0058] In a preferred embodiment, at least in the surface portion of the multi-metal material, the primary catalyst material, comprising Cu or consisting of Cu, is predominant. Thus, at least the surface portion of the multi-metal material comprises from 50 wt% to 99 wt% of the primary catalyst material, based on the total weight of the surface portion of the multi-metal material, preferably from 60 wt% to 98 wt% of the primary catalyst material, more preferably from 65 wt% to 97 wt% of the primary catalyst material, even more preferably from 70 wt% to 96 wt% of the primary catalyst material.

[0059] In a preferred embodiment, at least in the surface portion of the multi-metal material, the enhancer material, comprising Al or consisting of Al, is present in a weight percentage that is inferior to the weight percentage of the primary catalyst material. Thus, at least the surface portion of the multi-metal material comprises from 1 wt% to 50 wt% of the enhancer material, based on the total weight of the surface portion of the multi-metal material, preferably from 2 wt% to 40 wt% of the enhancer material, more preferably from 3 wt% to 35 wt% of the enhancer material, even more preferably from 4 wt% to 30 wt% of the enhancer material.

[0060] In a preferred embodiment, at least the surface region comprises an Al content of 1 wt% to 50 wt% and a Cu content of 50 wt% to 99 wt%, or comprises an Al content of 3 wt% to 30 wt% and a Cu content of 70 wt% to 97 wt%.

[0061] In a preferred embodiment, at least the surface region consists of Cu and Al; with preference, the multi-metal material consists of Cu and Al.

[0062] In a preferred embodiment, at least the surface region of the multi-metal material is nanoporous. In another embodiment, at least 50 wt% of the multi-metal material is nanoporous based on the total weight of the multi-metal material, preferably 95 wt% of the multi-metal material is nanoporous.

[0063] The multi-metal material comprises pores having a pore diameter ranging from 1 nm to 100 nm as determined by HRTEM and HAADF analysis, preferably from 2 nm to 80 nm; more preferably from 3 nm to 60 nm, even more preferably from 4 nm to 40 nm and most preferably from 5 nm to 20 nm.

[0064] In a preferred embodiment, at least the surface region has a homogeneous distribution of Al and Cu, which means that at least the Al on the surface region is uniformly distributed within the Cu-Al material, i.e. no aggregated metallic Al nanocluster or other metallic Al nanomorphology on the surface.

[0065] In an embodiment, the Cu in at least the surface region is Cu (100); with preference, the Al content in the Cu (100) is about 3 wt% to about 15 wt%

[0066] In another embodiment, the Cu in at least the surface region is Cu (111); with preference, the Al content in the Cu (111) is about 8 wt% to about 15 wt%, or about 11 wt% to about 13 wt%.

Method to manufacture the electrocatalyst

[0067] The electrocatalyst is preferably manufactured by physical vapour deposition and chemical etching processes. In another embodiment, the electrocatalyst is manufactured by ions implanting.

[0068] Methods of manufacturing Cu-Al based electrocatalysts have been developed and, in some implementations, use physical vapour deposition and chemical etching processes, which facilitates scalable fabrication of nanoporous Cu-Al catalysts. When manufactured by vapour deposition and chemical etching processes, the method comprises the following steps:

• producing a metallic material, i.e. a multi-metal material, comprising Cu and Al; and
• subjecting the metallic material; i.e. a multi-metal material, to chemical etching to remove a portion of the Al from a surface region of the metallic alloy to produce a de-alloyed multi-metal Cu-Al material.

[0069] The step of producing a metallic material, i.e. a multi-metal material, comprising Cu and Al preferably comprises vapour-phase deposition of Al onto a Cu surface; such as evaporating solid Al and forming a deposited Al layer on the Cu surface to form an evaporated Al-on-Cu material, wherein the deposited Al layer has a thickness ranging from 20 to 200 nm as determined by cross-sectional scanning electron microscopy, preferably from 50 to 150 nm, more preferably from 60 to 100 nm.

[0070] With preference, the step of evaporating of the solid Al is performed at an evaporation rate ranging from 1 to 10 nm s^-1, preferably from 1 to 5 nm s^-1, more preferably from 1 to 2 nm s^-1.

[0071] More preferably, the step of evaporating of the solid Al is performed under a base pressure ranging from 10^-5 to 10^-8 Torr i.e. 133.32 × 10^-5 to 133.32 × 10^-8 Pa.

[0072] According to the invention, the chemical etching comprises immersing the evaporated Al-on-Cu material into an acidic solution to remove Al.

[0073] With preference, the acidic solution comprises hydrochloric acid solution; preferably, the hydrochloric acid solution comprises from 1 to 20 wt% of hydrochloric acid based on the total weight of the hydrochloric acid solution, preferably from 1 to 18 wt%, more preferably from 1 to 15 wt%, even more preferably from 1 to 12 wt%, most preferably from 1 to 10 wt%, even most preferably from 1 to 8 wt% or from 1 to 5 wt% of hydrochloric acid.

[0074] Preferably, the method comprises, after chemical etching, washing with water to remove the acidic solution; with preference, the method further comprises, after washing, air drying to remove water.

[0075] In a preferred embodiment, the method further comprises, prior to producing the metallic alloy comprising the Cu and Al, depositing Cu on a gas diffusion layer (GDL); with preference, the Cu is deposited by thermal evaporation onto the GDL

[0076] Preferably, the Cu forms a deposited Cu layer on the GDL; wherein the deposited Cu layer has a thickness ranging from 300 to 1000 nm as determined by cross-sectional scanning electron microscopy, preferably from 350 to 800 nm, more preferably from 400 to 600 nm and even more preferably from 450 to 550 nm.

[0077] In an embodiment, the step of producing a multi-metal material comprising Cu and Al comprises co-evaporation of Al and Cu to form a Cu-Al alloy; with preference the multi-metal material comprising Cu and Al form a layer having a thickness ranging from 200 to 1000 nm as determined by cross-sectional scanning electron microscopy, preferably from 250 to 800 nm, more preferably from 300 to 500 nm.

[0078] With preference, the method further compris depositing a layer of the Cu-Al alloy onto a gas diffusion layer (GDL) prior to the chemical etching; more preferably, the method comprises cooling the deposited Cu-Al alloy prior to chemical etching.

[0079] With preference, the chemical etching comprises immersing the Cu-Al alloy in an acidic solution to remove Al; with preference, the acidic solution comprises hydrochloric acid solution. More preferably, after chemical etching, washing with water to remove the acidic solution.

[0080] In another embodiment the method of manufacturing an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, the method comprising ion-implanting Al into Cu. That is, a Cu catalyst layer is made with a desired thickness on a gas diffusion layer first, and then, Al is ion-implanted into Cu to make a Cu-Al surface.

[0081] In some implementations, the Cu-Al based electrocatalysts enable highly selective production of ethylene with a record CO₂-to-C₂H₄ Faradaic efficiency of 80% at an unprecedently high applied current density of 600 mA cm^-2 (-1.8 to -2.1 V vs. RHE) in a flow cell system. This result vastly improves the CO₂-to-C₂H₄ selectivity and stability with a fairly high half-cell electricity-to-ethylene power conversion efficiency of 30% which readily meets the requirements of practical operation. Embodiments of the de-alloyed nanoporous Cu-Al catalysts achieve a CO₂-to-C₂H₄ Faradaic efficiency of 80% at an applied current density of 600 mA cm^-2 with an applied cathodic potential between -1.8 to -2.1 V vs. RHE (corresponding to a full-cell voltage of 3.03 to 3.33 V in the ideal case considering a 1.23 V on the OER side).

[0082] The rapid increase in global energy demand and the need to replace fossil fuels with renewable sources necessitate vast chemical storage of intermittent solar and wind electricity. The electrochemical reduction of CO₂ to valuable chemical feedstocks represents a promising means of utilizing CO₂ and renewable energy combined. Until now, copper has been the predominant electrocatalyst for the production of multi-carbon products, but it has certain drawbacks.

[0083] Accelerated discovery of potential catalysts was performed. The results suggested that copper-rich Cu-Al alloys provide multiple sites and surface orientations that exhibit optimal CO adsorption energies near the top of the activity volcano plot for CO₂ reduction. Experimentally, the invention showed that incorporating, e.g., 4-28%, of Al on Cu surfaces increases their Faradaic efficiency (FE) in C₂H₄ electroproduction from about 35% (with pure Cu) to over 60% (with Al incorporated Cu).

[0084] The invention further developed a scalable physical vapour deposition and chemical etching process to fabricate nanoporous Cu-Al catalysts that electrochemically reduced CO₂ to C₂H₄ with a record FE of 80% at a current density of 600 mA cm^-2 (-1.8 to -2.1 V vs. RHE) in 1 M KOH electrolyte in a flow cell system. An average C₂H₄ FE of 75% ± 4% was obtained over 17 de-alloyed distinct Cu-Al samples under the same current density of 600 mA cm^-2.

[0085] In situ X-ray absorption revealed how Cu and Al enable a favourable Cu coordination environment that enhances C-C dimerization. The findings suggest new avenues by which multi-metallic systems can be devised that go beyond the limitations of conventional single-metal electrocatalysts.

[0086] It will be appreciated from the overall description and the experimentation section in particular that the catalyst materials, as well as the associated methods described herein, can have a number of optional features, variations, and applications.

EXAMPLES & EXPERIMENTATION

[0087] The present invention enabled accelerated discovery of Cu-Al motifs for highly active CO₂ electroreduction to ethylene.

[0088] While copper has been the predominant electrocatalyst for the production of multi-carbon products, analyses using Density Functional Theory (DFT) screened potential catalytic materials and suggested that copper-rich Cu-Al alloys provide multiple sites and surface orientations that exhibit optimal CO adsorption energies near the top of the activity volcano plot for CO₂ reduction. Experimentally, the invention shows that incorporating 4-28% of Al on Cu surfaces increases their Faradaic efficiency in C₂H₄ electroproduction. The invention further developed a simple and scalable physical vapour deposition and chemical etching process to fabricate nanoporous Cu-Al catalysts that electrochemically reduced CO₂ to C₂H₄ with a record Faradaic efficiency of 80% at a current density of 600 mA cm^-2 (-1.8 to -2.1 V vs. RHE) in 1 M KOH electrolyte in a flow cell system. In situ X-ray absorption reveals how Cu and Al enable a favourable Cu coordination environment that enhances C-C dimerization. The findings also suggest new avenues by which multi-metallic systems can be devised that go beyond the limitations of conventional single-metal electrocatalysts.

[0089] The invention prepared experimentally a suite of model catalysts to implement these recommended directions: ion-implanted Al-on-Cu and evaporated-etched Al-on-Cu (see Methods section and Fig. 8). Each catalyst shows a morphology similar to that of an evaporated pure Cu catalyst (see Fig. 9-11).

[0090] Compared with the pure Cu catalyst, which attained a C₂H₄ Faradaic efficiency (FE) of 35% at a current density of 600 mA cm^-2 in a 1 M KOH electrolyte in a flow-cell configuration (see Fig. 12), both ion-implanted and evaporated-etched Al-on-Cu catalysts exhibited higher C₂H₄ FEs of ~60% under the same testing conditions. The CO FEs on both Cu-Al catalysts were suppressed to ~10%, one-third of that obtained using pure Cu (see Fig. 13). Incorporating Al on Cu thus increased selectivity toward C₂H₄. Tafel slopes of C₂H₄ production (see Fig. 13) for pure Cu, ion-implanted, and evaporated-etched Al-on-Cu are 180, 147 and 145 mV dec^-1, respectively, further highlighting the faster C-C dimerization kinetics with Al-on-Cu catalysts.

[0091] To estimate quantitatively the amount of Al incorporated near the Cu surface, the invention used surface-sensitive Auger electron spectroscopic (AES) analysis (see Fig. 14, 15). AES typically provides compositional information on the top 1-3 nm of the samples and does so over a relatively large area (100 µm² in the experiments). The invention estimated Al concentrations on surfaces of 4.5% and 25% for the ion-implanted and evaporated-etched Al-on-Cu, respectively.

[0092] Pourbaix diagrams (see Fig. 16) show that both Cu and Al are cathodically protected at potentials more negative than their oxidation potentials of -1.4 V vs. RHE in a pH 14 electrolyte. This should enable their stable use as electrocatalysts in alkaline electrolytes.

[0093] The invention performed CO₂ electrolysis and achieved a remarkably high current density of 600 mA cm^-2 at a cathodic potential of -1.8 vs. RHE. The C₂H₄ FEs of the ion-implanted and evaporated-etched Al-on-Cu catalysts were stable at ~60% over operating periods of 5 hours before the failure of the gas diffusion electrode due to mechanical flooding. SEM and EDX analyses confirmed no major change of morphologies and Al concentrations before and after 5 hours of reaction (see Fig. 10, 11, 17-20; and Fig. 21-24).

[0094] The invention then sought to develop an optimized and robust catalyst combining Cu and Al. The invention explored vapour phase deposition followed by chemical etching wherein the inventors would synthesize de-alloyed nanoporous Cu-Al catalysts. As shown in the scanning electron spectroscopy (SEM) and high angle angular dark field-scanning transmission electron microscopy (HAADF-STEM) images in Fig. 2b and Fig. 25, a nanoporous structure with pore diameters of 5-20 nm was formed. Compared to ion-implanted and evaporated-etched Al-on-Cu catalysts, the de-alloyed nanoporous Cu-Al catalysts may offer more catalytically active sites for adsorption and electroreduction of CO₂ Following 5 hours CO₂ electroreduction at a current density of 600 mA cm^-2, the morphology remained similar indicating a stable catalyst and structure (Fig. 2b). The grain size of the catalyst increased following reaction, potentially due to the surface reconstruction of Cu and Al in the electrolyte during the reaction. Energy-dispersive X-ray spectroscopy (EDX) analyses in TEM and SEM, electron energy loss spectroscopy (EELS) spectra, and elemental mapping in STEM, all confirmed a homogeneous distribution of Al and Cu in de-alloyed catalysts before and following 5 hours reaction (Fig. 2c and Fig. 26-28). The invention performed HAADF-STEM analysis and found that Cu (111) and (200) facets were observed with interplanar spacings of 0.211 and 0.182 nm (Fig. 29). AES analysis further revealed ~9% Al on the surface following the reaction respectively (Fig. 30, 31).

[0095] Given the presence of Cu (111) and (100) surfaces, the invention further analyzed how the ratio of Al to Cu on these surfaces affects ΔE_co (Fig. 1). The resulting distributions (Fig. 3a and 3b) show that adding ~12% Al to the Cu (111) surface maximizes the density of sites with ΔE_co values near the optimum of -0.67 eV and that adding 4-12% Al maximizes the density of optimal sites for the Cu (100) surface.

[0096] The invention performed density functional theory (DFT) calculations over the best ML predicted structures to characterize the changes in energy barriers in the major steps during CO₂ reduction. The reaction energy in the rate-determining step of C-C bond-making decreased from 1.6 eV to 0.9 eV on Cu (111) and from 0.7 eV to 0.4 eV on Cu (100) with the benefit of Al incorporation (see Fig. 32 to Fig. 33). This is consistent with ML predictions of increased C2+ production with Al-containing Cu.

[0097] The DFT results further showed that the reaction energy barrier for forming HO(CH)CH, an intermediate of ethanol, is higher than that for forming CCH, an intermediate of C₂H₄ with Al-containing Cu. Water near the Al atoms may act as a proton donor for the electrochemical dehydration reduction of HOCCH to CCH instead of hydrogenation of HOCCH to HO(CH)CH. Thus, oft-produced alcohol is suppressed and the C₂H₄ production is promoted.

[0098] The invention tested the CO₂ electroreduction activity of de-alloyed Cu-Al catalysts with different Al concentrations on the surfaces. A high C2+/C1 ratio of ~30 was obtained with ~10% Al on the surface which is in line with the ML and DFT predictions (Fig. 34).

[0099] The invention then evaluated the CO₂ electroreduction performance of the de-alloyed Cu-Al catalysts with ~10% Al at the surfaces at current densities from 200 to 800 mA cm^-2 in 1 M KOH in flow cells (Fig. 4a and 4b). To quantify FEs for each product, the invention carried out CO₂ electroreduction in a chronopotentiometry mode. As shown In Fig. 4a, the invention achieved C₂H₄ FE of 80% at a current density of 600 mA cm^-2. This is a 2-fold increase compared to the 35% FE of pure Cu measured under the same conditions. An electricity-to-ethylene half-cell power conversion efficiency (PCE) of 30% was achieved (Fig. 35), which is similar to the previously published highest half-cell PCE of ~30% using a plasma-activated copper electrocatalyst with a C₂H₄ FE of 60% obtained at an applied current density of ~12 mA cm^-2.

[0100] An average C₂H₄ FE of 75% ± 4% was obtained over 17 de-alloyed distinct Cu-Al samples (~10% Al on the surfaces) under the same current density of 600 mA cm^-2. The overall C2+ product was 85%-90% when the invention used the de-alloyed Al-based catalyst, appreciably higher than that the 55-60% using the flat Cu catalyst (Fig. 4b and Fig. 13).

[0101] The best Cu-Al catalysts exhibited stable potentials between -1.8 and -2.1 V vs. RHE and a C₂H₄ FE of 75% over 5 hours of continuous operation at 600 mA cm^-2 (Fig. 4e).

[0102] To acquire local coordination information during CO₂ electroreduction, the invention performed in situ synchrotron X-ray absorption near-edge structure (XANES) analysis under these same testing conditions. Cu-O bonding was observable via both ex-situ and in situ XANES analyses with the de-alloyed Cu-Al catalyst before, during and after the reaction. The intensity of the in situ Cu-O peak is smaller than that of the ex situ ones, indicating Cu-O in the de-alloyed Cu-AI catalyst was partially reduced to Cu during the reaction. In contrast, no obvious Cu-O bonding was observed for the pure Cu during the ex-situ and in situ analyses under the same testing conditions (see Fig. 7). It is proposed that a mixture of Cu-Cu and Cu-O was formed in the de-alloyed Cu-Al catalysts during the reaction. This may contribute to the favourable coordination environment that accelerates C-C dimerization, as predicted via DFT.

[0103] The invention designed control catalysts-nanoporous Cu with a very limited amount of Al on the surface and having similar nanoporosity to that of the de-alloyed Cu-Al catalyst-to clarify the role of morphology (Fig. 36). AES analysis revealed that surface Al was decreased from 10% to 2-3% (Fig. 37). Considering the penetration depth of 1-3 nm in the AES, the surface Al concentration on nanoporous Cu should be lower than 2-3%. The C₂H₄ FE was decreased to 53% at the same current of 600 mA cm^-2 (Fig. 4a and Fig. 38). Linear sweep voltammetry (LSV) curves for evaporated Cu, nanoporous Cu and de-alloyed Cu showed no obvious reduction peaks (Fig. 4c), indicating that all catalysts were stable and not reduced to other species at negative potentials. Tafel analysis of evaporated Cu and nanoporous Cu gave slopes of 180 mV dec^-1 and 175 mV dec^-1 for C₂H₄ production, respectively, which were both larger than that of 120 mV dec^-1 with the de-alloyed Cu-Al (Fig. 4d). It can be concluded from the invention that incorporating Al on the Cu surface is crucial to promote C₂H₄ production.

[0104] The invention thus developed a new de-alloyed Cu-Al catalyst for highly selective CO₂ electroreduction to C₂H₄. The findings suggest avenues to multi-metal catalysts that outperform single-component catalysts by utilizing an intermediate-binding-optimization strategy for multi-carbon production via CO₂ electroreduction.

Methods

[0105] DFT calculations. The DFT calculations were performed using a VASP package in the Generalized Gradient Framework formulated by Perdew et al., including the PBE flavour of DFT and the projector augmented wave (PAW) method to account for core-valence interactions. The cutoff of kinetic energy for plane wave expansions was set to 400 eV and the reciprocal space was sampled by the Γ- centred Monkhorst-Pack scheme with a grid of 2 by 2 by 1. The Cu (111) and (100) surface slabs were constructed with three Cu layers using ASE (Atomic Simulation Environment) using the PBE-optimized lattice parameter with a vacuum layer of at least 15 Å.

[0106] Zero-point energies (ZPE), enthalpy and entropy contributions to free energies at room temperature (298.15 K) were calculated from vibrational modes of surface species using numerical six-point derivatives in VASP and ASE. Note that very low-frequency modes were obtained in some cases because the explicit water molecules are not properly constrained by the hydrogen bonding network presented in water bulk. Such low-frequency modes can cause unphysically large entropy contributions, so they were reset to a threshold value of 60 cm^-1 and excluded frequencies smaller than the threshold, corresponding to the acoustic translational mode of the six-member rings in water bulk.

[0107] For the surface reaction (i.e., A^∗ → B^∗), the change in Gibbs free energy at temperature T and 1 atmospheric pressure is given by:

where ΔE_rxn is the calculated reaction energy of A^∗ → B^∗. ΔH⁰(T) and ΔS⁰(T, P⁰) are the enthalpy and entropy differences between the initial and final states. In addition, ΔH⁰(T) gives the zero-point energy and the temperature dependence of enthalpy change at a standard pressure of 1 atm for adsorption of molecule A (here, it is room temperature of 298.15 K), which is given by:

where

and

is the enthalpy at the temperature T and a standard pressure of 1 atm for the translational, rotational, vibrational modes of the A.

and

are entropy contributions from the 3-D translational, 2-D rotational, vibrational modes.

Examples

Example 1: Preparation of evaporated Cu on gas diffusion layers (GDLs).

[0108] Cu was evaporated on the GDL (Fuel Cell Store, Sigracet 39 BC) by a thermal evaporation process. GDL is made of an air-brushed polytetrafluoroethylene (PTFE) on carbon nanoparticles layer as a conductive and hydrophobic layer atop a carbon fibre layer as a conductive and supporting layer. 0.5 g Cu foils were placed in a crucible inside the evaporation chamber (Edwards AUTO 360 Thermal Evaporator). A thin Cu layer (~ 500 nm) was deposited at an evaporation rate of approximately 1-2 nm s^-1 under a base pressure of 10^-6 Torr. GDLs were kept rotating at a slow speed of 50 rpm during evaporation.

Example 2: Preparation of ion-implanted Al-on-Cu on GDLs.

[0109] Evaporated Cu on GDL samples were used as substrates and placed in ion implantation chamber (50keV Aluminum Implantation at Western University). A 99.999% purity aluminium (Al) rod is installed in a copper target in the caesium (Cs) sputter source. A 100keV Al₂^- molecules are produced in the sputter source injector, selected by the injector magnet and injected into the Tandetron accelerator. Al₂^- is preferred because it has six times the flux of Al^- . For ion implants below 100keV, the Tandetron terminal pump and stripper gas are turned off. The Tandetron is used as a large lens to focus a negative beam to target in the implant chamber. The high energy magnet steers the Al₂^- down the beamline with the implant chamber. As the beam travels down the beamline it passes through NEC Electrostatic Raster/Scanner which sweeps the beam in the X direction at 517Hz and 64Hz in the Y direction over an aperture which defines the implant area on the implant stage. The Al₂^- molecule breaks into Al each having an energy of 50keV after the collisions with the sample. The implant stage has 4 sides. Each side can be rotated to face the beam for implantation. The implant stage in the Implant Chamber is suspended in a Faraday cage to suppress the secondary electrons. The ion charge is collected from the implant stage and fed to an Ortec 439 current integrator. The charge is converted into pulses which are counted by a computer to determine the dose. To avoid substantial ion-beam induced damage and over-heating to the samples, the inventors ion implanted 2 w% Al (a concentration compared to overall Cu) into Cu which corresponded to 6 × 10¹⁵ ions cm^-2. It took 112 minutes to finish this experiment. Auger electron spectroscopic analysis determined that the AI/(AI+Cu) molar concentration on the surface is ~4.5%. The inventors implanted 5 wt% and 10 wt% Al into Cu and it took 180 and 360 minutes, respectively. Surface Al concentrations are determined to be 5% and 5.5 %, indicating making more Al on Cu surface is difficult by the ion implantation method. This may be due to the ion-beam-induced damage and heating effect. Al may gradually migrate into the bulk at a large implantation dose.

Example 3: Preparation of evaporated-etched AI-on-Cu on GDLs.

[0110] Evaporated-etched Al-on-Cu was synthesized via a two-step process of evaporation and etching. First, 0.3 g Al foils were placed in a crucible inside the evaporation chamber. A thin Al layer (~ 100 nm) was deposited on evaporated Cu-on-GDL samples at an evaporation rate of approximately 1-2 nm s^-1 under a base pressure of 10^-6 Torr. The evaporated Al-on-Cu sample was then immersed in a 5 wt% hydrochloric acid solution to remove the excessive Al. The solution was kept stirring at a low speed of 250 rpm during the 5 minutes etching. Deionized water was used to wash off remained hydrochloric acid and other residual ions from the sample surface. An airbrush was used to dry the samples.

Example 4: Preparation of de-alloyed Cu-AI and nanoporous Cu on GDLs.

[0111] De-alloyed Cu-Al was synthesized via an evaporation and etching process. First, 0.5 g Cu foils and 0.25 g Al foils were placed in a crucible inside the deposition chamber. They were melted under a base pressure of 10^-6 Torr for 2 minutes to form greyish Cu-Al alloys. Then, a thin layer of Cu-Al alloy (~ 500 nm) was deposited on GDLs at an evaporation rate of approximately 1-2 nm s^-1 under a base pressure of 10^-6 Torr. After cooling down to room temperature naturally, the evaporated Cu-Al alloy on GDL samples were transferred to a 5 wt% hydrochloric acid solution to fabricate de-alloyed Cu-Al catalyst at a mild stirring speed of 250 rpm. Deionized water was used to wash off remained hydrochloric acid and other residual ions from the sample surface. An airbrush was used to carefully dry the samples.

[0112] Nanoporous Cu samples were prepared by immersing de-alloyed Cu-Al catalysts into 10 mM CuCl₂ solution for 10 minutes with a mild stirring speed of 50 rpm. Then, the samples were washed with deionized water and dried by an airbrush carefully.

[0113] Characterizations. The morphologies of the prepared samples were investigated using scanning electron microscope (SEM) on a Hitachi SU 5000 VPSEM, transmission electron microscope (TEM) on a Hitachi HF-3300 instrument with an acceleration voltage of 200kV and high-angle annular dark-field scanning transmission electron microscopy (HAADF-STEM) in a Cs-corrected STEM (JEOL, JEM-ARM200F) at an accelerating voltage of 200 kV. Compositions of the prepared samples were studied using Energy-dispersive X-ray spectroscopy (EDX) on a Bruker Quantax EDX in SEM and TEM, respectively, and electron energy loss spectroscopy (EELS) elemental analysis by GIF Quantum 965. Al concentrations on surfaces of the prepared samples were measured using Auger electron spectroscopy (AES) on a 710 Scanning Auger Nanoprobe instrument (Ulvac-PHI, Chigasaki, Japan). The beam settings used for the acquisition are 10keV and 10nA. AES analyses were performed at different locations on the surface for each sample to trace the Al concentrations and homogeneity. The inventors found that ion implantation gave rather uniform distributions of Al on the surfaces. In contrast, Al concentrations on those chemical etched samples may vary ± 5-10% especially for those samples with high Al concentrations, indicating that the chemical etching condition using HCl solutions might be further optimized.

[0114] Ex situ and in situ X-ray absorption spectra at Cu K-edge on catalysts and standard references were collected at the beamline of 1W1B from Beijing synchrotron radiation facility, China. The electron storage ring was operated at 2.5 GeV with an average current of 200 mA. A Si (111) double crystal was used as a monochromator and the data of absorption were collected in fluorescence mode. The energy of the absorption spectra was calibrated by measuring the X-ray absorption near edge spectroscopy (XANES) of a Cu metal foil. The obtained data were processed by established methods with the ATHENA software package. The normalized Extended X-ray absorption fine-structure spectroscopy (EXAFS) was converted from energy to k-space and weighted by k³. These data were then Fourier transformed to R-space.

[0115] For in situ measurements, a self-built flow cell consisting of two chambers for CO₂ diffusion (chamber I) and holding the reaction liquid (chamber II) was used. The sample is sandwiched between the two chambers with pressed the Teflon spacers (sample size: 1.2 × 1.2 cm²; thickness: ~500 nm). CO₂ gas is introduced into the chamber I with the gas controller and diffuses and passes through the samples and finally reaches the liquid to participate in the reaction. The thickness of the liquid can be controlled from 1000 to 200 µm. After the liquid cell filled with 1.0 M aqueous KOH, 30 mL KOH solution with the same concentration is flowed into the liquid cell at 0.5 mL/min by using an automatic pump syringe. The measurement of the Cu K-edge is started simultaneously with the stop of the flowing.

Example 5: Electrochemical reduction of CO₂.

[0116] All CO₂ electrolysis experiments were performed using a three-electrode set-up in a flow-cell configuration connected to an electrochemical workstation (Autolab PGSTAT302N). An Ag/AgCI (in saturated KCl solution) and a platinum wire were used as reference and counter electrodes, respectively. 1M KOH was used as the electrolyte. To quantify FEs for each product, CO₂ electrolysis was performed in a chronopotentiometry mode. For Tafel analysis, CO₂ electrolysis was performed in a Chronoamperometry mode. For linear sweep voltammogram (LSV) analyses, the LSV was cycled until it was stable.

[0117] The cathodic chamber was separated from the gas chamber by a 1.5 cm × 1.5 cm gas diffusion electrode (GDE). GDEs were made of catalysts on GDLs as discussed in detail above. A plastic plate with a 1cm × 1cm window is placed between the GDE and cathode chamber. The cathodic chamber was separated from the anodic chamber by an anion exchange membrane (Fumasep FAA-3-PK-130). Rubber spacers were placed in between different chambers to avoid mixture of electrolytes or gaseous products.

[0118] CO₂ gas was delivered into the gas chamber at a rate of 56 standard cubic centimetres per minute (s.c.c.m.) and was routed into a gas chromatograph (Perkin Elmer Clarus 680) to quantify the gaseous products. The liquid products were quantified by NMR (600 MHz Agilent DD2 spectrometer), in which electrolyte was mixed with D2O (deuterated water) and dimethyl sulfoxide (DMSO, Sigma, 99.99%) was used as an internal standard.

[0119] Faradaic efficiencies (FEs) for different products can be calculated as follows: FE = F × m × n / Q = F × m × n / (l × t), where F is the Faraday constant, m is the electron numbers needed for one CO₂ molecule reduction to the desired product and n is the amount of the desired product (in moles).

Example 6: The stability of Al for CO₂ electroreduction under our testing condition

[0120] To further test the electrochemical stability of Al, the invention performed a control experiment of electroreducing CO₂ using a pure Cu catalyst in 1 M KOH solution in the presence of 1 mM Al(OH)₄^- anions. Energy-dispersive X-ray spectroscopy (EDX) analysis showed ~4% Al after 30 minutes of CO₂ electroreduction at 600 mA cm^-2 (Fig. 21). AES analysis confirmed over 80% Al on the surface, indicating electrodeposition of Al (Fig. 22). Thus, the reverse reaction of dissolving Al into the solution to form Al(OH)₄^- anions was avoided. However, C₂H₄ production activity suffered at the expense of dramatically increased H₂ production (Fig. 23), highlighting the importance of realizing a homogeneous distribution of Al on Cu surface. As another control, a pure Cu electrode was immersed in the same solution of 1 M KOH and 1 mM Al(OH)₄^- for half hour without applying electrical bias. Al concentration was below EDX detection limit (Fig. 24).

Example 7: In situ and ex situ X-ray absorption studies.

[0121] A large amount of Cu-O bonding was visible continuously in the ex situ and in situ XANES analyses with the de-alloyed Cu-Al catalyst before, during and after the reaction (Fig. 7). In situ Fourier transform extended X-ray absorption fine structure (FT EXAFS) spectra of the de-alloyed Cu-Al catalysts, together with ex-situ reference spectra of Cu foil, Cu₂O and CuO, gave precise coordination information. The invention observed a prominent peak at ~2.2 Å from Cu-Cu contribution, which agrees with the prominent peak of Cu-Cu in Cu foils, and a weak peak at ~1.5 Å, which agrees with the prominent peak of Cu-O in Cu₂O and CuO. Moreover, the Cu-O peak intensity remained almost the same during in situ synchrotron measurement. It is smaller than that obtained with the same sample without CO₂ electroreduction (Fig. 7), indicating Cu-O in de-alloyed Cu-AI catalysts was partially reduced to Cu. A stable balance of Cu-Cu and Cu-O in the de-alloyed catalyst was established within a short time right after starting CO₂ electroreduction. As a control, the invention measured in situ XANES with a pure Cu on GDL under the same condition. No obvious oxidation state of Cu was observed (Fig. 7).

[0122] Data, findings and information from the present invention are also presented in the Figures and in the following tables:

Table 1: Zero-point energy and specific heat of different reactants, intermediates and products on the Al incorporated Cu (111) surface.

Structure	E_ZPE(eV)	Cv_trans(0->T)(eV)	Cv_rot(0->T)(eV)	Cv_vib(0->T)(eV)	H(eV)
Intial	2.17E+00	3.90E-02	3.90E-02	3.30E-01	2.61E+00
Finala	2.62E+00	3.90E-02	3.90E-02	4.30E-01	3.16E+00
Finalb	2.15E+00	3.90E-02	3.90E-02	3.77E-01	2.63E+00

Table 2: Entropy and Gibbs free energy of different reactants, intermediates and products on the Al incorporated Cu (111) surface.

Structure	S_trans(eV/K)	S_rot(eV/K)	S_vib(eV/K)	S(eV/K)	TS(eV)
Intial	2.19E-03	2.04E-03	2.08E-03	6.32E-03	1.88E+00
Finala	2.19E-03	2.00E-03	2.78E-03	6.97E-03	2.08E+00
Finalb	2.19E-03	2.03E-03	6.68E-03	6.68E-03	1.99E+00

Table 3: Zero-point energy and specific heat of different reactants, intermediates and products on the Al incorporated Cu (100) surface.

Structure	E_ZPE(eV)	Cv_trans(0->T)(eV)	Cv_rot(0->T)(eV)	Cv_vib(0->T)(eV)	H(eV)
Intial	2.15E+00	3.90E-02	3.90E-02	1.88E-01	2.44E+00
Finala	2.43E+00	3.90E-02	3.90E-02	1.82E-01	2.71E+00
Finalb	1.97E+00	3.90E-02	3.90E-02	1.76E-01	2.25E+00

Table 4: Entropy and Gibbs free energy of different reactants, intermediates and products on the Al incorporated Cu (100) surface.

Structure	S_trans(eV/K)	S_rot(eV/K)	S_vib(eV/K)	S(eV/K)	TS(eV)
Intial	2.17E-03	1.87E-03	1.17E-03	5.21E-03	1.55E+00
Finala	2.17E-03	1.87E-03	1.11E-03	5.14E-03	1.53E+00
Finalb	2.17E-03	1.87E-03	1.08E-03	5.12E-03	1.53E+00

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Claims

1. An electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, characterized in that the electrocatalyst comprises a multi-metal material comprising a primary metal being copper and at least one enhancer metal being aluminium, so the electrocatalyst comprises a multi-metal Cu-Al material being formed as a catalytic layer and comprises a surface region having a thickness between 1 nm and 3 nm as determined by Auger electron spectroscopy and in that at least the surface region is nanoporous and comprises an Al content of 3 wt% to 30 wt% and a Cu content of 70 wt% to 97 wt%.

2. The electrocatalyst according to claim 1, characterized in that the multi-metal Cu-Al material is a de-alloyed material.

3. The electrocatalyst according to claim 1 or 2, characterized in that the multi-metal Cu-AI material:

- comprises from 1 wt% to 50 wt% of Al based on the total weight of the multi-metal Cu-Al material, preferably from 3 wt% to 30 wt%; and /or

- comprises from 50 wt% to 99 wt% Cu based on the total weight of the multi-metal Cu-Al material, preferably from 70 wt% to 97 wt% Cu.

4. The electrocatalyst according to any one of claims 1 to 3, characterized in that the electrocatalyst comprises a gas diffusion membrane.

5. The electrocatalyst according to any one of claims 1 to 4, characterized in that the catalytic layer has a thickness between 10 nm and 5000 nm as determined by cross-sectional scanning electron microscopy.

6. The electrocatalyst according to any one of claims 1 to 5, characterized in that:

- the multi-metal Cu-Al material comprises Al-terminated pores; or

- the Al is ion-implanted into the Cu.

7. The electrocatalyst according to any one of claims 1 to 5, characterized in that the Al is present in the Cu as Al that has been evaporated into the Cu and remains after chemically etching; with preference, at least the surface region has pores that have pore diameters ranging from 1 nm to 100 nm as determined by HRTEM and HAADF analysis, or from 5 nm to 20 nm.

8. The electrocatalyst of any one of claims 1 to 7, characterized in that at least the surface region has a homogeneous distribution of Al and Cu; and/or at least the surface region consists of Cu and Al.

9. The electrocatalyst of any one of claims 1 to 8, characterized in that the Cu in at least the surface region is Cu (111); with preference, the Al content in the Cu (111) is about 8 wt% to about 15 wt%, or about 11 wt% to about 13 wt%.

10. The electrocatalyst of any one of claims 1 to 8, characterized in that the Cu in at least the surface region is Cu (100); with preference, the Al content in the Cu (100) is about 3 wt% to about 15 wt%.

11. Use of the electrocatalyst as defined in any one of claims 1 to 10 for electrocatalytic reduction of CO₂ into at least one multi-carbon compound; with preference, the electrocatalytic reduction of CO₂ is performed in a three-electrode flow-cell.

12. A process for electrochemical production of a multi-carbon compound from CO₂, comprising:

- contacting CO₂ gas and an electrolyte with an electrode comprising the electrocatalyst as defined in any one of claims 1 to 10, such that the CO₂ contacts the electrocatalyst;

- applying a voltage to provide a current density to cause the CO₂ gas contacting the electrocatalyst to be electrochemically converted into the multi-carbon compound; and

- recovering the multi-carbon compound.

with preference, the target multi-carbon compound is ethylene or an alcohol.

13. A system for CO₂ electroreduction to produce multi-carbon hydrocarbons for use in a process according to claim 12, comprising:

- an electrolytic cell configured to receive a liquid electrolyte and CO₂ gas;

- an anode;

- a cathode comprising an electrocatalyst as defined in any one of claims 1 to 10; and

- a voltage source to provide a current density to cause the CO₂ gas contacting the electrocatalyst to be electrochemically converted into the multi-carbon hydrocarbon, which is optionally ethylene or an alcohol.

14. A method of manufacturing an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, the method comprising:

- producing a multi-metal material comprising Cu and Al; and

- subjecting the multi-metal material to chemical etching to remove a portion of the Al from a surface region of the metallic alloy to produce a de-alloyed Cu-Al material.

wherein the electrocatalyst is according any one of claim 1 to 10.

15. A method of manufacturing an electrocatalyst for reduction of CO₂ to produce multi-carbon compounds, the method comprising ion-implanting Al into Cu wherein the electrocatalyst is according any one of claim 1 to 10.

Ansprüche

1. Elektrokatalysator zur Reduktion von CO₂ zur Produktion von Multikohlenstoffverbindungen, dadurch gekennzeichnet, dass der Elektrokatalysator ein Multimetallmaterial umfasst, welches ein Primärmetall, das Kupfer ist, und mindestens ein Verstärkermetall, das Aluminium ist, umfasst, so dass der Elektrokatalysator ein Multimetall-Cu-Al-Material umfasst, das als katalytische Schicht gebildet ist und eine Oberflächenregion mit einer Dicke zwischen 1 nm und 3 nm umfasst, bestimmt mittels Auger-Elektronenspektroskopie, und dass mindestens die Oberflächenregion nanoporös ist und einen Al-Gehalt von 3 Gew.% bis 30 Gew.% und einen Cu-Gehalt von 70 Gew.% bis 97 Gew.% umfasst.

2. Elektrokatalysator nach Anspruch 1, dadurch gekennzeichnet, dass das Multimetall-Cu-Al-Material ein entlegiertes Material ist.

3. Elektrokatalysator nach Anspruch 1 oder 2, dadurch gekennzeichnet, dass das Multimetall-Cu-Al-Material:

- 1 Gew.% bis 50 Gew.% Al, bezogen auf das Gesamtgewicht des Multimetall-Cu-Al-Materials, vorzugsweise 3 Gew.% bis 30 Gew.% umfasst; und/oder

- 50 Gew.% bis 99 Gew.% Cu, bezogen auf das Gesamtgewicht des Multimetall-Cu-Al-Materials, vorzugsweise 70 Gew.% bis 97 Gew.% umfasst.

4. Elektrokatalysator nach einem der Ansprüche 1 bis 3, dadurch gekennzeichnet, dass der Elektrokatalysator eine Gasdiffusionsmembran umfasst.

5. Elektrokatalysator nach einem der Ansprüche 1 bis 4, dadurch gekennzeichnet, dass die katalytische Schicht eine Dicke zwischen 10 nm und 5000 nm hat, bestimmt mittels Querschnitt-Rasterelektronenmikroskopie.

6. Elektrokatalysator nach einem der Ansprüche 1 bis 5, dadurch gekennzeichnet, dass:

- das Multimetall-Cu-Al-Material Poren mit endständigem Al umfasst; oder

- das Al in das Cu ionenimplantiert ist.

7. Elektrokatalysator nach einem der Ansprüche 1 bis 5, dadurch gekennzeichnet, dass das Al in dem Cu als Al vorliegt, das in das Cu eingedampft wurde und nach chemischem Ätzen verbleibt; wobei bevorzugt mindestens die Oberflächenregion Poren aufweist, die Porendurchmesser im Bereich von 1 nm bis 100 nm, bestimmt gemäß HRTEM- und HAADF-Analyse, oder von 5 nm bis 20 nm haben.

8. Elektrokatalysator nach einem der Ansprüche 1 bis 7, dadurch gekennzeichnet, dass mindestens die Oberflächenregion eine homogene Verteilung von Al und Cu hat; und/oder mindestens die Oberflächenregion aus Cu und Al besteht.

9. Elektrokatalysator nach einem der Ansprüche 1 bis 8, dadurch gekennzeichnet, dass das Cu in mindestens der Oberflächenregion Cu (111) ist; wobei der Al-Gehalt in dem Cu (111) vorzugsweise etwa 8 Gew.% bis etwa 15 Gew.% oder etwa 11 Gew.% bis etwa 13 Gew.% beträgt.

10. Elektrokatalysator nach einem der Ansprüche 1 bis 8, dadurch gekennzeichnet, dass das Cu in mindestens der Oberflächenregion Cu (100) ist; wobei der Al-Gehalt in dem Cu (100) vorzugsweise etwa 3 Gew.% bis etwa 15 Gew.% beträgt.

11. Verwendung des Elektrokatalysators, wie in einem der Ansprüche 1 bis 10 definiert, für elektrokatalytische Reduktion von CO₂ zu mindestens einer Multikohlenstoffverbindung; wobei die elektrokatalytische Reduktion von CO₂ vorzugsweise in einer Flusszelle mit drei Elektroden durchgeführt wird.

12. Verfahren zur elektrochemischen Produktion einer Multikohlenstoffverbindung aus CO₂, umfassend:

- Kontaktieren von CO₂-Gas und einem Elektrolyten mit einer Elektrode, die den Elektrokatalysator wie in einem der Ansprüche 1 bis 10 definiert umfasst, so dass das CO₂ den Elektrokatalysator kontaktiert;

- Anlegen einer Spannung, um eine Stromdichte bereitzustellen, um zu bewirken, dass das CO₂-Gas, welches den Elektrokatalysator kontaktiert, elektrochemisch in die Multikohlenstoffverbindung konvertiert wird; und

- Gewinnen der Multikohlenstoffverbindung,

wobei die angestrebte Multikohlenstoffverbindung bevorzugt Ethylen oder ein Alkohol ist.

13. System für CO₂-Elektroreduktion, um Multikohlenstoffkohlenwasserstoffe zur Verwendung in einem Verfahren gemäß Anspruch 12 zu produzieren, umfassend:

- eine Elektrolysezelle, die ausgestaltet ist, um einen flüssigen Elektrolyten und CO₂-Gas zu empfangen;

- eine Anode;

- eine Kathode, umfassend einen Elektrokatalysator wie in einem der Ansprüche 1 bis 10 definiert; und

- eine Spannungsquelle, um eine Stromdichte bereitzustellen, um zu bewirken, dass das CO₂-Gas, welches den Elektrokatalysator kontaktiert, elektrochemisch in den Multikohlenstoff-Kohlenwasserstoff, der gegebenenfalls Ethylen ist, oder einen Alkohol konvertiert wird.

14. Verfahren zur Fertigung eines Elektrokatalysators zur Reduktion von CO₂ zur Produktion von Multikohlenstoffverbindungen, wobei das Verfahren umfasst:

- Produzieren eines Multimetallmaterials, das Cu und Al umfasst; und

- Unterziehen des Multimetallmaterials chemischem Ätzen, um einen Anteil an Al aus einer Oberflächenregion der metallischen Legierung zu entfernen, um ein entlegiertes Cu-Al-Material zu produzieren, wobei der Elektrokatalysator gemäß einem der Ansprüche 1 bis 10 ist.

15. Verfahren zur Fertigung eines Elektrokatalysators zur Reduktion von CO₂, um Multikohlenstoffverbindungen zu produzieren, wobei das Verfahren Ionenimplantieren von Al in Cu umfasst, wobei der Elektrokatalysator gemäß einem der Ansprüche 1 bis 10 ist.

Revendications

1. Électrocatalyseur pour la réduction du CO₂ afin de produire des composés multicarbonés, caractérisé en ce que l'électrocatalyseur comprend un matériau multimétallique comprenant un métal primaire étant le cuivre et au moins un métal activateur étant l'aluminium, de sorte que l'électrocatalyseur comprend un matériau multimétallique Cu-Al étant formé en tant que couche catalytique et comprend une région de surface ayant une épaisseur entre 1 nm et 3 nm telle que déterminée par spectroscopie électronique Auger et en ce qu'au moins la région de surface est nanoporeuse et comprend une teneur en Al de 3 % en poids à 30 % en poids et une teneur en Cu de 70 % en poids à 97 % en poids.

2. Électrocatalyseur selon la revendication 1, caractérisé en ce que le matériau multimétallique Cu-Al est un matériau désallié.

3. Électrocatalyseur selon la revendication 1 ou 2, caractérisé en ce que le matériau multimétallique Cu-Al :

- comprend de 1 % en poids à 50 % en poids d'AI sur la base du poids total du matériau multimétallique Cu-Al, de préférence de 3 % en poids à 30 % en poids ; et/ou

- comprend de 50 % en poids à 99 % en poids de Cu sur la base du poids total du matériau multimétallique Cu-Al, de préférence de 70 % en poids à 97 % en poids de Cu.

4. Électrocatalyseur selon l'une quelconque des revendications 1 à 3, caractérisé en ce que l'électrocatalyseur comprend une membrane de diffusion de gaz.

5. Électrocatalyseur selon l'une quelconque des revendications 1 à 4, caractérisé en ce que la couche catalytique a une épaisseur comprise entre 10 nm et 5000 nm telle que déterminée par microscopie électronique à balayage en coupe.

6. Électrocatalyseur selon l'une quelconque des revendications 1 à 5, caractérisé en ce que :

- le matériau multimétallique Cu-Al comprend des pores terminés par Al ; ou

- l'AI est implanté par ions dans le Cu.

7. Électrocatalyseur selon l'une quelconque des revendications 1 à 5, caractérisé en ce que l'Al est présent dans le Cu sous forme d'Al évaporé dans le Cu et restant après la gravure ; de préférence, au moins la région de surface a des pores ayant des diamètres de pores allant de 1 nm à 100 nm comme déterminé par analyse HRTEM et HAADF, ou de 5 nm à 20 nm.

8. Électrocatalyseur selon l'une quelconque des revendications 1 à 7, caractérisé en ce qu'au moins la région de surface a une répartition homogène de Al et Cu ; et/ou au moins la région de surface est constituée de Cu et d'Al.

9. Électrocatalyseur selon l'une quelconque des revendications 1 à 8, caractérisé en ce que le Cu dans au moins la région de surface est Cu (111) ; de préférence, la teneur en Al dans le Cu (111) est d'environ 8 % en poids à environ 15 % en poids, ou d'environ 11 % en poids à environ 13 % en poids.

10. Électrocatalyseur selon l'une quelconque des revendications 1 à 8, caractérisé en ce que le Cu dans au moins la région de surface est Cu (100) ; de préférence, la teneur en Al dans le Cu (100) est d'environ 3 % en poids à environ 15 % en poids.

11. Utilisation de l'électrocatalyseur tel que défini selon l'une quelconque des revendications 1 à 10 pour la réduction électrocatalytique du CO₂ en au moins un composé multicarboné ; de préférence, la réduction électrocatalytique du CO₂ est effectuée dans une cellule de débit à trois électrodes.

12. Procédé de production électrochimique d'un composé multicarboné à partir de CO₂, comprenant :

- la mise en contact du gaz CO₂ et un électrolyte avec une électrode comprenant l'électrocatalyseur tel que défini selon l'une quelconque des revendications 1 à 10, de sorte que le CO₂ entre en contact avec l'électrocatalyseur ;

- l'application d'une tension pour fournir une densité de courant afin d'amener le gaz CO₂ en contact avec l'électrocatalyseur à être converti électrochimiquement en composé multicarboné ; et

- la récupération du composé multicarboné.

de préférence, le composé multicarboné cible est l'éthylène ou un alcool.

13. Système pour une électroréduction du CO₂ pour produire des hydrocarbures multicarbonés destinés à être utilisés dans un procédé selon la revendication 12, comprenant :

- une cellule électrolytique configurée pour recevoir un électrolyte liquide et du gaz CO₂ ;

- une anode ;

- une cathode comprenant un électrocatalyseur tel que défini selon l'une quelconque des revendications 1 à 10 ; et

- une source de tension pour fournir une densité de courant afin d'amener le gaz CO₂ en contact avec l'électrocatalyseur à être converti électrochimiquement en l'hydrocarbure multicarboné, qui est optionnellement de l'éthylène ou un alcool.

14. Méthode de fabrication d'un électrocatalyseur pour la réduction du CO₂ afin de produire des composés multicarbonés, la méthode comprenant les étapes consistant à :

- produire un matériau multimétallique comprenant du Cu et de l'Al ; et

- soumettre le matériau multimétallique à une gravure pour éliminer une partie de l'AI d'une région de surface de l'alliage métallique afin de produire un matériau Cu-AI désallié,

dans laquelle l'électrocatalyseur est selon l'une quelconque des revendications 1 à 10.

15. Méthode de fabrication d'un électrocatalyseur pour la réduction du CO₂ afin de produire des composés multicarbonés, la méthode comprenant l'implantation d'ions Al dans Cu, dans laquelle l'électrocatalyseur est selon l'une quelconque des revendications 1 à 10.

Drawing